baby's spoon with a surface area of 6.25 cm? is plated with silver from AGNO, using a current of 2 A for two hours d 25 minutes. How many grams of silver are plated? What is the thickness of the silver plate formed? (density of silver =10.5 g/cm)

Q: Simply by living, an 87.5 kg human being will consume approximately 20.0 mol of 0, per day. To…

A:

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: Faraday's first law of electrolysis states that the mass of substance deposited is directly…

Q: How many grams of silver can be plated onto an object in 9.87 minutes at 4.74 A of current ?…

A:

Q: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

A:

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

Q: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

A:

Q: A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5in x 8.5in x…

A: first we have to find the volume,volume=length ×width×heightthen we know,density=massvolumeby…

Q: Simply by living, an 87.5 kg human being will consume approximately 20.0 mol of 0, per day. To…

A: The answer is given below :

Q: What mass of gold can be plated onto an object in 9.18 minutes at 4.91 A of current ? Au^3^+…

A:

Q: 6. A 1M aqueous solution of chromium (I) bromide will be electrolyzed to "chrome plate" a faucet.…

A: As per the Faraday's 1st law of electrolysis: w=ZIt      ----(1)where,w = weight of the substance…

Q: n a copper plating experiment in which copper metal is deposited from a copper(II) ion solution, the…

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: A battery can provide a current of 2.20 A at 1.00 V for 8.00 hr. How much energy (in kJ) is…

A: Given information,Battery provides a current 2.20 A at 1.00 V for 8.00 hr.Calculate the power,

Q: A current of 3.86 A is passed through a Pb(NO,), solution for 1.60 h. How much lead is plated out of…

A: Faraday law of electrolysis states that the amount of substance deposited at the electrode is…

Q: A current of 4.15 A is passed through a Pb(NO3)2 solution for 1.50 h. How much lead is plated out of…

A: Given that:  Current(I) = 4.15A = 4.15C/s  Time(t) = 1.50h = 1.50h×3600s/h = 5400s Reaction:  Pb2+ +…

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The electrical energy which is generated in the lead storage battery will be equivalent to the…

Q: An electrolysis cell that deposits gold (from Au*(a)) operates for 15 minutes at a current of 2.30…

A:

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

A:

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction:

Q: A solution containing a metal ion (M2+ (aq)) is electrolyzed by a current of 7.8 A. After 15.5…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: When a lead storage battery is recharged by a current of 12.0 A for 15 minutes, what mass of PbSO4…

A: The given data contains,     I =12 A    Time (t)=15 min x60 s=900 Seconds

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

Q: Gold can be plated out of a solution containing Au3+ according to the half-reaction:Au3+(aq) + 3…

A: It is given that gold is plated for 25 minutes and the current is of 5.5 A and the half-reaction is…

Q: What mass of zinc is required to galvanize the top of a 3.00 m × 5.50 m sheet of iron to a thickness…

A: Given: Thickness =0.100mm=0.0001m area of the sheet=3.00m×5.50m current=2.25A Density of…

Q: What mass of platinum could be plated on an electrode from the electrolysis of a Pt4+ (aq) solution…

A: The given data contains, Current =0.500 ATime =55 smolar mass ofPt=55 g/mol Charge =+4

Q: How much silver would fall out of a solution of AgNO3 if a current of 5.00 amperes passed through it…

A: Given,  Current = I = 5.00 A  Time period = t = 2 hours  How much silver would fall out of a…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: 4.) What mass of silver can be plated onto an object in 45 minutes at 9.0 A of current?

A:

Q: Question attached

A: Current is equal to the flow of charge per unit of time. It is denoted by I. Its SI unit is ampere.…

Q: A battery can provide a current of 2.20 A at 1.40 V for 10.0 hr. How much energy (in kJ) is…

A: GIVEN: Current = 2.20 A Voltage = 1.40 V Time= 10.0 hr To CALCULATE: Energy (kJ)

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A:

Q: Many "muscle" car enthusiasts like to use chrome-plated engine parts when restoring a muscle car of…

A: Mass of Chromium =  m = 25 gMolar Mass of Chromium = 52 g/molNo of moles of Chromium = n = m Mn = 25…

Q: A gold (III) chloride solution was electrolyzed using a current of 13.5 amperes for four hours. How…

A: Mass deposit or plated  = Z.i.t

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: Electrolysis is a process in which current is passed through a substance .In this chemical reactions…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: The electrochemical reaction of silver is –

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

Q: What mass of aluminum can be plated onto an object in 378 minutes at 5.80 A of current?…

A: A numerical problem based on Faraday's law, which is to be accomplished.

Q: decided to deposit 55.00 g of gold over an iron medallion by electroplating it from a solution…

A:

Q: What current in ampere will be required to produce 2.369 x10-3 kg of cu from CuSO4 solution in one…

A: Required mass of Cu to be produced = 2.369×10-3 Kg = 2.369 g Time given = 1 Hour = 1×60×60 = 3600…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 5.1…

A: Solution: From the Faraday first law we have, the amount of chemical change being produced by a…

Q: How many minutes are required to deposit 3.77 g Cr from a Cr³⁺(aq) solution

A: We will calculate time for deposit of metal

Q: How many coulombs of charge pass through a cell if 3.0 amperes of current are passed through the…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: A digital watch battery draws 0.10 milliamperes of current, which is provided by a mercury battery…

A: m=Mass of Hg=1.10g Equivalent wt of Hg =200.59/2 =100.295 Current = 0.10 mA or 0.10x10-3 F=96500C…

Q: How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

A: Amount of the current flow = 20A Mass of liberated substance = 10g Electron transfer per ion = 3

Q: A digital watch battery draws 0.35 milliamperes of current, which is provided by a mercury battery…

A: The moles of HgO and Zn can be calculated as -

Q: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge  i.e  Q = i x t  Where  Q= charge in coulombs  i = current  in…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.